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Sequence of Chemical Reactions—Student Laboratory Kit

By: The Flinn Staff

Item #: AP5605

Price: $63.25

In Stock.

In the Sequence of Chemical Reactions Laboratory Kit, start with copper, and end with copper! Students practice filtering, decanting, precipitating, and neutralizing as they perform this amazing chemical feat.

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Product Details

Start with copper—end with copper! Students perform a series of chemical reactions to convert copper metal to its nitrate, hydroxide, oxide, chloride, phosphate, sulfate and finally... back to copper metal. Students practice many standard laboratory techniques, such as filtering, decanting, precipitating and neutralizing as they perform this amazing chemical feat. For each reaction in the cycle, students write a balanced chemical equation, note physical states of products, learn reaction types and calculate percent yield.

Complete for 30 students working in pairs. Perform this experiment in a fume hood or well-ventilated lab. Entire lab may take 3–5 laboratory periods.

Specifications

Materials Included in Kit: 
Copper turnings, 10 g
Hydrochloric acid solution, 6 M, 250 mL
Nitric acid solution, 8 M, 100 mL
Sodium hydroxide solution, 8 M, 250 mL
Sodium phosphate solution, 0.3 M, 300 mL
Sulfuric acid solution, 2 M, 250 mL, 2
Zinc, mossy, 60 g
Filter paper, 12.5 cm, pkg/50
Foil barrier bag, 4½" x 3" x 12" x 4.3 mil nylon, 2
Hydrion® 1–12 pH test strips, vial of 100
Pipet, Beral-type, thin stem, 100


Correlation to Next Generation Science Standards (NGSS)

Science & Engineering Practices

Analyzing and interpreting data
Developing and using models
Constructing explanations and designing solutions

Disciplinary Core Ideas

MS-PS1.A: Structure and Properties of Matter
MS-PS1.B: Chemical Reactions
HS-PS1.B: Chemical Reactions

Crosscutting Concepts

Patterns
Energy and matter

Performance Expectations

MS-PS1-2. Analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred.
MS-PS1-5. Develop and use a model to describe how the total number of atoms does not change in a chemical reaction and thus mass is conserved.
HS-PS1-2. Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.